SOME BASIC CONCEPTS OF CHEMISTRY
One point one. IMPORTANCE OF CHEMISTRY
One point two. NATURE OF MATTER
SOME BASIC CONCEPTS OF CHEMISTRY
One point Three. Properties of Matter and Their Measurement
One point Three point one. The International System of Units
Some Basic Concepts of Chemistry
One point Three point two. Mass and Weight
Maintaining the National Standards of Measurement
Some Basic Concepts of Chemistry
One point four UNCERTAINTY IN MEASUREMENT
One point four point one Scientific Notation
SOME BASIC CONCEPTS OF CHEMISTRY
Multiplication and Division
One point four point two Significant Figures
Multiplication and Division of Significant Figures
One point four point three Dimensional Analysis
SOME BASIC CONCEPTS OF CHEMISTRY
One point five point two Law of Definite Proportions
One point five point three Law of Multiple Proportions
One point five point four Gay Lussac's Law of Gaseous Volumes
One point five point five Avogadro Law
SOME BASIC CONCEPTS OF CHEMISTRY
One point six DALTON'S ATOMIC THEORY
One point seven ATOMIC AND MOLECULAR MASSES After having some idea about the terms atoms and molecules, it is appropriate here to
One point seven point one Atomic Mass
One point seven point three Molecular Mass
One point seven point four Formula Mass
SOME BASIC CONCEPTS OF CHEMISTRY
One point nine PERCENTAGE COMPOSITION
One point nine point one Empirical Formula for Molecular Formula.
SOME BASIC CONCEPTS OF CHEMISTRY
One point ten STOICHIOMETRY AND
One point ten point one. Limiting Reagent
SOME BASIC CONCEPTS OF CHEMISTRY
One point ten point two. Reactions in Solutions
Let us now study each one of them in detail. One. Mass per cent
SOME BASIC CONCEPTS OF CHEMISTRY
One point two. Calculate the mass per cent of different elements present in sodium sulphate (Na two SO four).
One point seven. How much copper can be obtained from one hundred grams of copper sulphate?
One point nine. Calculate the atomic mass (average) of chlorine using the following data:
One point fourteen. What is the SI unit of mass? How is it defined?
SOME BASIC CONCEPTS OF CHEMISTRY
Two point one SUB-ATOMIC PARTICLES
Two point one point one Discovery of Electron
Two point one point two Charge to Mass Ratio of Electron
Millikan's Oil Drop Method
Two point two Atomic Models
Two point two point one Thomson Model of Atom
Two point two point four Isobars and Isotopes.
Two point two point five Drawbacks of Rutherford Model.
Two point three Developments Leading to the Bohr's Model of Atom
Two point three point one Wave Nature of Electromagnetic Radiation
Two point three point two Particle Nature of Electromagnetic Radiation: Planck's Quantum Theory
Dual Behaviour of Electromagnetic Radiation
Two point three point three Evidence for the quantized Electronic Energy Levels: Atomic spectra
Emission and Absorption Spectra
Line Spectrum of Hydrogen
Two point four Bohr's Model for Hydrogen Atom
Two point four point one Explanation of Line Spectrum of Hydrogen
equals three point two nine times ten to the fifteenth
Two point four point two Limitations of Bohr's Model
Two point five Towards Quantum Mechanical Model of the Atom
Two point five point one Dual Behaviour of Matter
Problem two point thirteen
Significance of Uncertainty Principle
Problem two point fifteen
Two point six QUANTUM MECHANICAL MODEL OF ATOM
Hydrogen Atom and the Schrödinger Equation
Important Features of the Quantum Mechanical Model of Atom
Orbit, orbital and its importance
Problem two point seventeen
Problem two point eighteen
Two point six point three Energies of Orbitals
Two point six point four Filling of Orbitals in Atom
Pauli Exclusion Principle
Two point six point six Stability of Completely Filled and Half Filled Subshells
Two point three How many neutrons and protons are there in the following nuclei ?
Two point four Write the complete symbol for the atom with the given atomic number (Z) and atomic mass (A)
Two point twenty-two. Which of the following are isoelectronic species i.e., those having the same number of electrons?
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
Three point one. Why do we need to classify elements?
Classification of elements and periodicity in properties
Classification of elements and periodicity in properties
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
Three point four NOMENCLATURE OF ELEMENTS WITH ATOMIC NUMBERS GREATER THAN ONE HUNDRED
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
Three point five ELECTRONIC CONFIGURATIONS OF ELEMENTS AND THE PERIODIC TABLE
(a) Electronic Configurations in Periods
Three point six ELECTRONIC CONFIGURATIONS AND TYPES OF ELEMENTS: s-, p-, d-, f- BLOCKS
Three point six point one The s-Block Elements
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
Three point six point two The p-Block Elements
Three point six point three The d-Block Elements (Transition Elements)
Three point six point four The f-Block Elements (Inner-Transition Elements)
Problem three point three
Three point seven Periodic Trends in Properties of Elements
Three point seven point one Trends in Physical Properties
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
(d) Electron Gain Enthalpy
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
Three point seven point two Periodic Trends in Chemical Properties
(a) Periodicity of Valence or Oxidation States
Problem three point eight
(b) Anomalous Properties of Second Period Elements
Three point seven point three Periodic Trends and Chemical Reactivity
CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
Three point nineteen. The first ionization enthalpy values (in kilojoules per mole) of group thirteen elements are:
Three point twenty. Which of the following pairs of elements would have a more negative electron gain enthalpy? (i) Oxygen or fluorine (ii) For chlorine
Three point twenty-seven. Use the periodic table to answer the following questions.
Chemical Bonding and Molecular Structure
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point one point one Octet Rule
Four point one point two Covalent Bond
Chemical Bonding and Molecular Structure
Four point one point three Lewis Representation of Simple Molecules (the Lewis Structures)
Four point one point four Formal Charge
Chemical Bonding and Molecular Structure
Four point one point five Limitations of the Octet Rule
Other drawbacks of the octet theory
Four point two. IONIC OR ELECTROVALENT BOND
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point two point one Lattice Enthalpy
Four point three BOND PARAMETERS
Four point three point two Bond Angle
Four point three point three Bond Enthalpy
Four point three point four Bond Order
Four point three point five Resonance Structures
Four point three point six Polarity of Bonds
Four point four. The Valence Shell Electron Pair Repulsion Theory
Chemical Bonding and Molecular Structure
Chemical Bonding and Molecular Structure
Four point five. Valence Bond Theory
Four point five point one. Orbital Overlap Concept
Chemical Bonding and Molecular Structure
Four point five point three. Overlapping of Atomic Orbitals
Four point five point four. Types of Overlapping and Nature of Covalent Bonds
Four point five point five. Strength of Sigma and pi Bonds
Four point six. Hybridisation
Salient features of hybridisation: The main features of hybridisation are as under :
Chemical Bonding and Molecular Structure
Important conditions for hybridisation
Four point six point one. Types of Hybridisation
Example of molecule having sp hybridisation
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point six point three Hybridisation of Elements involving d Orbitals
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point seven MOLECULAR ORBITAL THEORY
Four point seven point one Formation of Molecular Orbitals Linear Combination of Atomic Orbitals (LCAO)
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point seven point two Conditions for the Combination of Atomic Orbitals
Four point seven point three Types of Molecular Orbitals
Four point seven point four Energy Level Diagram for Molecular Orbitals
CHEICAL BONDING AND MOLECULAR STRUCTURE
Four point seven point five Electronic Configuration and Molecular Behaviour
Four point eight Bonding in some homonuclear diatomic molecules
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point nine point one Cause of Formation of Hydrogen Bond
Four point nine point two Types of H-Bonds
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point two. Write Lewis dot symbols for atoms of the following elements: Magnesium, Sodium, Boron, Oxygen, Nitrogen, Bromine.
Four point four. Draw the Lewis structures for the following molecules and ions:
Four point five. Define octet rule. Write its significance and limitations.
Four point nine. How do you express the bond strength in terms of bond order?
Four point thirteen. Write the resonance structures for Sulfur trioxide, Nitrogen dioxide, and Nitrate one.
Four point sixteen. Write the significance or applications of dipole moment.
Four point twenty-four. What is meant by hybridization of atomic orbitals? Describe the shapes of S P, S P two, S P three hybrid orbitals.
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Four point thirty-one. What do you understand by bond pairs and lone pairs of electrons? Illustrate by giving one example of each type.
Four point thirty-three. Explain the formation of Hydrogen molecule on the basis of valence bond theory.
Four point thirty-five. Use molecular orbital theory to explain why the Beryllium two molecule does not exist.
Four point thirty-seven. Write the significance of a plus and a minus sign shown in representing the orbitals.
Four point thirty-nine. Define hydrogen bond. Is it weaker or stronger than the van der Waals forces?
Five point one INTERMOLECULAR FORCES
Five point one point two Dipole - Dipole Forces
Five point one point three Dipole-Induced Dipole Forces
Five point one point four Hydrogen bond
Five point two. Thermal Energy
Five point three. Intermolecular Forces and Thermal Interactions
Five point four. The Gaseous State
Five point five. The Gas Laws
Five point five point one. Boyle's Law (Pressure - Volume Relationship)
Five point five point two. Charles' Law (Temperature - Volume Relationship)
Five point five point three Gay Lussac's Law (Pressure-Temperature Relationship)
Five point five point four Avogadro Law (Volume-Amount Relationship)
Five point six Ideal Gas Equation
Five point six point one Density and Molar Mass of a Gaseous Substance
Five point six point two Dalton's Law of Partial Pressures
Five point seven KINETIC MOLECULAR THEORY OF GASES
Five point eight. Behaviour of Real Gases: Deviation from Ideal Gas Behaviour
Five point nine LIQUIFACTION OF GASES
Five point ten LIQUID STATE
Five point ten point one Vapour Pressure
Five point ten point two Surface Tension
Five point ten point three Viscosity
Six point one. THERMODYNAMIC STATE
Six point one point one. The System and the Surroundings
Six point one point two. Types of the System
Six point one point three. The State of the System
Six point one point four. The Internal Energy as a State Function
Six point two Applications
Six point two point one Work
Isothermal and free expansion of an ideal gas
(b) Extensive and Intensive Properties
one mole of the substance and is the quantity of heat needed to raise the temperature of one mole by one degree Celsius (or one Kelvin). Specific heat, also called specific heat capacity is the quanti
(d) The relationship between C sub v and C sub p for an ideal gas
Six point three MEASUREMENT OF delta U AND delta H: CALORIMETRY
Six point four ENTHALPY CHANGE, AH OF A REACTION - REACTION ENTHALPY
(a) Standard enthalpy of reactions
(b) Enthalpy changes during phase transformations
(d) Thermochemical equations
(e) Hess's Law of Constant Heat Summation
Six point five ENTHALPIES FOR DIFFERENT TYPES OF REACTIONS
(a) Standard enthalpy of combustion (symbol: Delta H naught)
(b) Enthalpy of atomization (symbol: Delta sub a H naught)
(c) Bond Enthalpy (symbol: Delta sub bond H naught)
(d) Enthalpy of Solution (symbol: A H nano)
Ionization Energy and Electron Affinity
Six point six SPONTANEITY.
(a) Is decrease in enthalpy a criterion for spontaneity ?
(b) Entropy and spontaneity.
(c) Gibbs energy and spontaneity
Six point seven Gibbs energy change and equilibrium
Six point thirteen. Given
Seven point one. Equilibrium in physical processes
Seven point one point one. Solid-Liquid Equilibrium
Seven point one point two. Liquid-Vapour Equilibrium
Seven point one point three Solid - Vapour Equilibrium
Seven point one point four Equilibrium Involving Dissolution of Solid or Gases in Liquids
Seven point two EQUILIBRIUM IN CHEMICAL PROCESSES - DYNAMIC EQUILIBRIUM
Dynamic Equilibrium - A Student's Activity
Seven point three LAW OF CHEMICAL EQUILIBRIUM AND EQUILIBRIUM CONSTANT
Seven point four HOMOGENEOUS EQUILIBRIA
Seven point four point one Equilibrium Constant in Gaseous Systems
Problem seven point three
Seven point five HETEROGENEOUS EQUILIBRIA
Units of Equilibrium Constant
Seven point six APPLICATIONS OF EQUILIBRIUM CONSTANTS
Seven point six point two. Predicting the Direction of the Reaction.
Problem seven point seven
Seven point six point three Calculating Equilibrium Concentrations
Problem seven point eight
Partial pressures at equilibrium are,
Seven point seven RELATIONSHIP BETWEEN EQUILIBRIUM CONSTANT K, REACTION QUOTIENT Q AND GIBBS ENERGY G
Seven point eight point one Effect of Concentration Change
Effect of Concentration - An experiment This can be demonstrated by the following reaction:
Seven point eight point two. Effect of Pressure Change
Seven point eight point three. Effect of Inert Gas Addition
Seven point eight point four. Effect of Temperature Change
Seven point eight point five Effect of a Catalyst
Seven point nine IONIC EQUILIBRIUM IN SOLUTION
Seven point ten ACIDS, BASES AND SALTS
Seven point ten point one. Arrhenius Concept of Acids and Bases
Hydronium and Hydroxyl Ions
Seven point ten point two. The Brönsted-Lowry Acids and Bases
Problem seven point fourteen
Seven point eleven Ionization of Acids and Bases
Seven point eleven point one. The Ionization Constant of Water and its Ionic Product
Seven point eleven point two. The pH Scale
Problem seven point eighteen
Problem seven point one nine
Problem seven point two zero
Seven point one one point four Ionization of Weak Bases
Problem seven point two one
Problem seven point two two
Seven point one one point five Relation between K sub a and K sub one
Problem seven point two three
Seven point one one point six Di- and Polybasic Acids and Di- and Polyacidic Bases
Seven point eleven point seven Factors Affecting Acid Strength
Seven point eleven point eight Common Ion Effect in the Ionization of Acids and Bases
Seven point eleven point nine Hydrolysis of Salts and the P H of their Solutions
Problem seven point two five
Seven point one three SOLUBILITY EQUILIBRIA OF SPARINGLY SOLUBLE SALTS
Seven point one three point one Solubility Product Constant
Problem seven point two six
Problem seven point twenty-seven
Seven point thirteen point two Common Ion Effect on Solubility of Ionic Salts
Problem seven point twenty-eight
SUGGESTED ACTIVITIES FOR STUDENTS REGARDING THIS UNIT
Answer to Some Selected Problems